GCSE SCIENCE (Double Award) 1
GCSE in SCIENCE (Double Award) (Wales)
Summary of Assessment
There are two tiers of entry for this qualification:
Higher Tier – Grades A* - D
Foundation Tier – Grades C - G
Y9&Y10
Unit 1: (Double Award) BIOLOGY 1
Written examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
Unit 2: (Double Award) CHEMISTRY 1
Written examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
Unit 3: (Double Award) PHYSICS 1
Written examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
Unit 4: (Double Award) BIOLOGY 2
Written examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
2.2 Unit 2
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GCSE SCIENCE (Double Award) 2
(Double Award) CHEMISTRY 1
Written examination: 1 hour 15 minutes 15% of qualification
This unit includes the following topics:
2.1
The nature of substances and chemical reactions
2.2
Atomic structure and the Periodic Table
2.3
Water
2.4
The ever-changing Earth
2.5
Rate of chemical change
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GCSE SCIENCE (Double Award) 3
2.1 THE NATURE OF SUBSTANCES AND CHEMICAL REACTIONS
elements as substances that cannot be broken down into simpler substances by chemical
means and as the basic building blocks of all substances
elements as substances made up of only one type of atom
compounds as substances made of two or more different types of atom that are chemically
joined and having completely different properties to its constituent elements
how to represent elements using chemical symbols and simple molecules using chemical
formulae
how to represent simple molecules using a diagram and key
how to write the formulae of ionic compounds given the formulae of the ions they contain
relative atomic mass and relative molecular (formula) mass
the percentage composition of compounds
atoms/molecules in mixtures not being chemically joined and mixtures being easily
separated by physical processes such as filtration, evaporation, chromatography and
distillation
chromatographic data analysis and Rf values
chemical reactions as a process of re-arrangement of the atoms present in the reactants to
form one or more products, which have the same total number of each type of atom as the
reactants
colour changes, temperature changes (exothermic/endothermic) and effervescence as
evidence that a chemical reaction has taken place
how to represent chemical reactions using word equations
how to represent chemical reactions using balanced chemical equations where the total
relative mass of reactants and products is equal
the percentage yield of a chemical reaction
how to calculate the formula of a compound from reacting mass data
how to calculate the masses of reactants or products from a balanced chemical equation
the Avogadro constant and the mole and how to convert amount of substance in grams to
moles and vice versa
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GCSE SCIENCE (Double Award) 4
2.2 ATOMIC STRUCTURE AND THE PERIODIC TABLE
atoms containing a positively charged nucleus with orbiting negatively charged electrons
atomic nuclei containing protons and neutrons
the relative masses and relative charges of protons, neutrons and electrons
atoms having no overall electrical charge
the terms atomic number, mass number and isotope
how the numbers of protons, neutrons and electrons present in an atom are related to its
atomic number and mass number
elements being arranged in order of increasing atomic number and in groups and periods in
the modern Periodic Table, with elements having similar properties appearing in the same
groups
metals being found to the left and centre of the Periodic Table and non-metals to the right,
with elements having intermediate properties appearing between the metals and nonmetals in each period
the electronic structures of the first 20 elements
how the electronic structure of any element is related to its position in the Periodic Table
the similarities and trends in physical and chemical properties of elements in the same
group as illustrated by Group 1 and Group 7
many reactions, including those of Group 1 elements and many of those of Group 7
elements, involve the loss or gain of electrons and the formation of charged ions
the trends in reactivity of Group 1 and Group 7 elements in terms of their readiness to
lose or gain an electron
the reactions of the alkali metals with air/oxygen, the halogens and water
the test used to identify hydrogen gas
the reactions of halogens with alkali metals and with iron
the relative reactivities of chlorine, bromine and iodine as demonstrated by displacement
reactions
the properties and uses of chlorine and iodine
the identification of Li+, Na+, K+, Ca2+ and Ba2+ ions by flame tests and Cl‒, Br‒ and I‒ ions by
their reactions with silver nitrate solution (including ionic equations)
the unreactive nature of the Group 0 gases and the uses of helium, neon and argon
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GCSE SCIENCE (Double Award) 5
2.3 WATER
the composition of water in ‘natural’ water supplies, including dissolved gases, ions,
microorganisms and pollutants
the need for a sustainable water supply to include reducing our water consumption,
reducing the environmental impacts of abstracting, distributing and treating water
the treatment of the public water supply using sedimentation, filtration and chlorination
the arguments for and against the fluoridation of the water supply in order to prevent tooth
decay
desalination of sea water to supply drinking water including the sustainability of this
process on a large scale
the separation of water and other miscible liquids by distillation
simple methods to determine solubility and produce solubility curves
the interpretation of solubility curves
the causes of hardness in water and how to distinguish between hard and soft waters by
their action with soap
the difference between temporary and permanent hardness
the processes used to soften water to include boiling, adding sodium carbonate and ion
exchange; the advantages and disadvantages of different methods of water softening and
the explanation of how these methods work
the health benefits of hard water and its negative effects, e.g. on boiler elements
SPECIFIED PRACTICAL WORK
 Determination of the amount of hardness in water using soap solution
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GCSE SCIENCE (Double Award) 6
2.4 THE EVER-CHANGING EARTH
the large scale structure of the Earth in terms of solid iron core, molten iron outer core,
mantle and crust
the theory of plate tectonics and how it developed from Alfred Wegener's earlier theory of
continental drift
the processes occurring at conservative, destructive and constructive plate boundaries
where plates slide past one another, move towards one another and move apart
respectively
the formation of the original atmosphere by gases, including carbon dioxide and water
vapour, being expelled from volcanoes
the present composition of the atmosphere and how the composition of the atmosphere
has changed over geological time
the roles of respiration, combustion and photosynthesis in the maintenance of the levels of
oxygen and carbon dioxide in the atmosphere
the environmental effects and consequences of the emission of carbon dioxide and sulfur
dioxide into the atmosphere through the combustion of fossil fuels
the measures used to address the problems of global warming and acid rain
the air as a source of nitrogen, oxygen, neon and argon
the tests used to identify oxygen gas and carbon dioxide gas
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GCSE SCIENCE (Double Award) 7
2.5 RATE OF CHEMICAL CHANGE
practical methods used to determine the rate of reaction – gas collection, loss of mass and
precipitation (including using data-logging apparatus)
the effect of changes in temperature, concentration (pressure) and surface area on rate of
reaction
the particle theory in explaining changes of rate as a result of changes in temperature,
concentration (pressure) and surface area
catalysts as substances that increase the rate of a reaction while remaining chemically
unchanged and that they work by lowering the energy required for a collision to be
successful (details of energy profiles are not required)
SPECIFIED PRACTICAL WORK
 Investigation of the factors that affect the rate of a reaction using a gas collection method
 Investigation of the factors that affect the rate of the reaction between dilute hydrochloric acid and
sodium thiosulfate
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GCSE SCIENCE (Double Award) 8
2.5 Unit 5 (Double Award) CHEMISTRY 2
Written examination: 1 hour 15 minutes 15% of qualification
This unit includes the following topics:
5.1
Bonding, structure and properties
5.2
Acids, bases and salts
5.3
Metals and their extraction
5.4
Chemical reactions and energy
5.5
Crude oil, fuels and carbon compounds
NOTE
All content relating to formulae and equations and calculations based upon them (specified in Unit 2.1) is
required for Unit 5. All chemical tests specified in Unit 2 are required for Unit 5.
Unit 5: (Double Award) CHEMISTRY 2
Written examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
Unit 6: (Double Award) PHYSICS 2
Written Examination: 1 hour 15 minutes
15% of qualification
60 marks
A mix of short answer questions, structured questions, extended writing and data response questions
with some set in a practical context. A tiered assessment.
Unit 7: (Double Award) PRACTICAL ASSESSMENT
10% of qualification
60 marks
Practical assessment that will be carried out in centres, but will be externally marked by WJEC. It will take
place in the first half of the spring term (January – February). It is
recommended that this should be in the final year of study. An untiered assessment.
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GCSE SCIENCE (Double Award) 9
5.1
BONDING, STRUCTURE AND PROPERTIES
the properties of metals, ionic compounds, simple molecular covalent substances and
giant covalent substances
the 'sea' of electrons/lattice of positive ions structural model for metals in explaining
their physical properties
electronic structure in explaining how ionic bonding takes place (and how this is
represented using dot and cross diagrams)
the accepted structural model for giant ionic structures in explaining the physical
properties of ionic compounds
electronic structure in explaining how covalent bonds are formed (and how this is
represented using dot and cross diagrams)
the intermolecular bonding structural model for simple molecular structures in
explaining the physical properties of simple molecular substances
the properties of diamond, graphite, fullerenes, carbon nano-tubes and graphene and
how these are explained in terms of structure and bonding
individual atoms not having the same properties as bulk materials as demonstrated by
diamond, graphite, fullerenes, carbon nano-tubes and graphene having different
properties despite all containing only carbon atoms, and by nano-scale silver particles
exhibiting properties not seen in bulk silver
the properties and uses of nano-scale particles of silver and titanium dioxide
the possible risks associated with the use of nano-scale particles of silver and titanium
dioxide, and of potential future developments in nanoscience
the properties and uses of smart materials including thermochromic pigments,
photochromic pigments, polymer gels, shape memory alloys and shape memory polymers
5.2
ACIDS, BASES AND SALTS
Overview
substances as acidic, alkaline or neutral in terms of the pH scale, including acid/alkali
strength
solutions of acids containing hydrogen ions and alkalis containing hydroxide ions
the reactions of dilute acids with metals and how these relate to the metals' position in
the reactivity series
the neutralisation of dilute acids with bases (including alkalis) and carbonates
neutralisation as the reaction of hydrogen ions with hydroxide ions to form water
H+(aq) + OH‒(aq) → H2O(l)
the acid/carbonate reaction as a test for acidic substances and CO32‒ ions
the preparation of crystals of soluble salts, such as copper(II) sulfate, from insoluble
bases and carbonates
the names of the salts formed by hydrochloric acid, nitric acid and sulfuric acid
the test used to identify SO42‒ ions
titration as a method to prepare solutions of soluble salts and to determine relative
concentrations of solutions of acids/alkalis
SPECIFIED PRACTICAL WORK
 Preparation of crystals of a soluble salt from an insoluble base or carbonate
 Titration of a strong acid against a strong base using an indicator
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GCSE SCIENCE (Double Award) 10
5.3 METALS AND THEIR EXTRACTION
ores found in the Earth's crust as the source of most metals and that these metals can be
extracted using chemical reactions
some unreactive metals (e.g. gold) being found in their native form and that the difficulty
involved in extracting metals increases as their reactivity increases
the relative reactivities of metals as demonstrated by displacement (e.g. iron nail in
copper(II) chloride solution) and competition reactions (e.g. thermit reaction)
reduction and oxidation in terms of removal or gain of oxygen
the industrial extraction of iron in the blast furnace, including the combustion, reduction,
decomposition and neutralisation reactions
electrolysis of molten ionic compounds e.g. lead(II) bromide (including electrode
equations)
reduction and oxidation in terms of gain or loss of electrons
the industrial extraction of aluminium using electrolysis, including the use of cryolite to
dissolve alumina
the properties and uses of iron (steel), aluminium, copper and titanium
the general properties of transition metals, including their ability to form ions with
different charges
an alloy being a mixture made by mixing molten metals, whose properties can be
modified by changing its composition
factors affecting economic viability and sustainability of extraction processes
e.g. siting of plants, fuel and energy costs, greenhouse emissions and recycling
SPECIFIED PRACTICAL WORK
 Determination of relative reactivities of metals through displacement reactions
5.4 CHEMICAL REACTIONS AND ENERGY
exothermic and endothermic reactions in terms of temperature change and energy
transfer to or from the surroundings
energy profiles for exothermic and endothermic reactions
the activation energy as the energy needed for a reaction to occur
the use of bond energy data to calculate overall energy change for a reaction and to
identify whether it is exothermic or endothermic
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GCSE SCIENCE (Double Award) 11
5.5 CRUDE OIL, FUELS AND CARBON COMPOUNDS
crude oil as a complex mixture of hydrocarbons that was formed over millions of years
from the remains of simple marine organisms
the fractional distillation of crude oil
fractions as containing mixtures of hydrocarbons (alkanes) with similar boiling points
the trends in properties of fractions with increasing chain length and the effect on their
usefulness as fuels
the global economic and political importance and social and environmental impact of the
oil industry
the combustion reactions of hydrocarbons and other fuels
how to determine experimentally the energy per gram released by a burning fuel
the combustion reaction of hydrogen and its use as an energy source including its
advantages and disadvantages as a fuel
the fire triangle in fire-fighting and fire prevention
the cracking of some fractions to produce smaller and more useful hydrocarbon
molecules, including monomers (alkenes) which can be used to make plastics
the general formula CnH2n+2 for alkanes and CnH2n for alkenes
the names and molecular and structural formulae for simple alkanes and alkenes
isomerism in more complex alkanes and alkenes
the addition reactions of alkenes with hydrogen and bromine and the use of bromine
water in testing for alkenes
the addition polymerisation of ethene and other monomers to produce polythene,
poly(propene), poly(vinylchloride) and poly(tetrafluoroethene)
the general properties of plastics and the uses of polythene, poly(propene),
poly(vinylchloride) and poly(tetrafluoroethene)
the environmental issues relating to the disposal of plastics, in terms of their nonbiodegradability, increasing pressure on landfill for waste disposal, and how recycling
addresses these issues as well as the need to carefully manage the use of finite natural
resources such as crude oil
SPECIFIED PRACTICAL WORK
 Determination of the amount of energy released by a fuel
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